Calculate E_cell for an Electrochemical Cell Based on the Two $\to$

question 155

Multiple Choice

Calculate E_cell for an electrochemical cell based on the two half-reactions given below when the reaction occurs in an acidic aqueous solution in which the pH is buffered at 4.00 and [MnO₄^-] = 1.80 M and [Fe²⁺] = 0.0220 M.Use the smallest whole-number coefficients possible when balancing the overall reaction. MnO₄^- + 4 H⁺ + 3e^- $\to$ MnO₂ + 2 H₂O $\quad$ +1.673 V
Fe²⁺ + 2 e^- $\to$ Fe $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ -0.447 V

• A)+2.10 V
• B)+0.964 V
• C)+1.21 V
• D)+1.86 V
• E)+2.38 V

Outline the process and requirements for the formal adoption of the U.S. Constitution.

Describe the motivations and desired outcomes behind the control of interstate commerce and finance by the national government.

Understand the debate and reasoning surrounding the addition of a Bill of Rights to the Constitution.

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